Onsider the following reaction at equilibrium: CO(g) + Cl2(g)COCl2(g) Predict whether the reaction will shift left, shift right, or remain the unchanged upon each of the following disturbances. a) COCl2 is added to thereaction mixtureb) Cl2 is added to thereaction mixturec) COCl2 is removed fromthe reaction mixture

Explanation:

CO(g) + Cl2(g) ⇄ COCl2(g)

This question is based on Le Chatelier's principle.

Le Chatelier's principle is an observation about chemical equilibria of reactions. It states that changes in the temperature, pressure, volume, or concentration of a system will result in predictable and opposing changes in the system in order to achieve a new equilibrium state.

a) COCl2 is added to the reaction mixture

COCL2 is a product in the reaction. If we add additional product to a system, the equilibrium will shift to the left, in order to produce more reactants. The reaction would shift to the left.

b) Cl2 is added to the reaction mixture

if we add reactants to the system, equilibrium will be shifted to the right to in order to maintain equilibrium by producing more products.

c) COCl2 is removed from the reaction mixture

if we remove products from the system, equilibrium will be shifted to the right to in order to maintain equilibrium by producing more products.